Diluting Solutions to Prepare Workable Solutions

Basically in this lesson we learnt how to dilute solutions to prepare solutions you can actually work with.
We need to be able to make solutions of any concentration.
The equation is actually pretty easy:

Formula: M₁L₁ = M₂L₂

_{What this means is the amount moles of the solute before is equal to how many moles of solute there are after.}

_{The subscript 1 = before}

The subscript 2 = after

Just a little note: Final Volume - Before Volume = Water Added

Example

We have 100 mL of 0.125 M H2SO4. We want to end up with 0.500 M H2SO4. 

HOW DO YOU DO IT?

So remember the formula from above. 

Step 1.

100 mL of 0.125 M --> 0.500 M

100 mL x 0.125 M = mL x 0.500 M

Step 2. 

You have to separate the mL so that it is away from the equation , like you do in algebra.

100 mL x 0.125 M = mL

                                                            0.500 M 

Step 3.

Basically all you have to do is calculate.

Once you've calculated it all you'll get something like this: 

25 = mL.

So you will need 25 mL of H2SO4 to get 0.500 M of H2SO4.

So easy, right?

Key Concepts

• The concentration of a solution is usually given in moles per litre (mol/L). 
• This is also known as molarity.
• Concentration, or Molarity, is given the symbol M. 
• The solute is the substance which dissolves.
• The solvent is the liquid which does the dissolving.
• A solution is prepared by dissolving a solute in a solvent.
• When a solution is diluted, more solvent is added to it.

Can you imagine drinking lemonade without it being diluted first? It'd be pure lemon! Yuck!

Lemonade is made by adding around 4 cups of water to a concentrated solution of lemon.

Without the water it'd just be a really sour syrup! How good can that taste?

If you STILL don't understand, check out this video

How to Dilute a Solution